1. III. Periodic Trends (p. 140 - 154)
Ch. 5 - The Periodic Table
III. Periodic Trends (p )

2. A. Periodic Law
When elements are arranged in order of increasing atomic #, elements with similar properties appear at regular intervals.

3. B. Chemical Reactivity Families
Similar valence e- within a group result in similar chemical properties

4. B. Chemical Reactivity Alkali Metals Alkaline Earth Metals
Transition Metals
Halogens
Noble Gases

5. C. Other Properties Atomic Radius size of atom First Ionization Energy
© 1998 LOGAL
First Ionization Energy
Energy required to remove one e- from a neutral atom.
© 1998 LOGAL
Melting/Boiling Point

6. D. Atomic Radius
Atomic Radius K Na Li Ar Ne

7. D. Atomic Radius
Atomic Radius
Increases to the LEFT and DOWN

8. D. Atomic Radius Why larger going down?
Higher energy levels have larger orbitals
Shielding – core (inner) e- block the attraction between the nucleus and the valence e-
Why smaller to the right?
Increased nuclear charge without additional shielding pulls e- in tighter

9. E. Ionization Energy
First Ionization Energy He Ne Ar Li Na K

10. E. Ionization Energy First Ionization Energy
Increases UP and to the RIGHT

11. E. Ionization Energy Why opposite of atomic radius?
In small atoms, e- are close to the nucleus where the attraction is stronger
Why small jumps within each group?
Stable e- configurations don’t want to lose e-

12. E. Ionization Energy Successive Ionization Energies
Large jump in I.E. occurs when a CORE e- is removed.
Mg 1st I.E kJ
2nd I.E. 1,445 kJ
Core e- 3rd I.E. 7,730 kJ

13. E. Ionization Energy Successive Ionization Energies
Large jump in I.E. occurs when a CORE e- is removed.
Al 1st I.E kJ
2nd I.E. 1,815 kJ
3rd I.E. 2,740 kJ
Core e- 4th I.E. 11,600 kJ

14. F. Melting/Boiling Point
Highest in the middle of a period.

15. G. Ionic Radius Ionic Radius Cations (+) lose e- smaller Anions (–)
gain e-
larger
© 2002 Prentice-Hall, Inc.

16. H. Electronegativity
*The measure of how strongly an atom attracts electrons when it is combined with another element
Increases from left to right (except for noble gases)
Increases as you move up a group

17. Examples
Which atom has the larger radius?
Be or Ba
Ca or Br Ba Ca

18. Examples
Which atom has the higher 1st I.E.?
N or Bi
Ba or Ne N Ne

19. Li or C Cr or Kr C Cr Examples
Which atom has the higher melting/boiling point?
Li or C
Cr or Kr C Cr

20. S or S2- Al or Al3+ S2- Al Examples
Which particle has the larger radius?
S or S2-
Al or Al3+
S2- Al